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UNIVERSITY  OF  ILLINOIS  BULLETIN 

Vol.  1  JULY  15.  1904  No.  20 


Published  Fortnig-htly  by  the  University  and  entered  at  Urbana,  Illinois,  as  second-class  matter 


Vol  1  JULY.  i9o4  No.  7 


The  Coals  of  Illinois;  Their  Composition 

and  Analysis 


s.  w.  parr,  m,  s.. 

Professor  of  Applied  Chemistry  in  the  University  of  Illinois 


THE  ILLINOIS  COMMISSION 
TO  THE  LOUISIANA  PURCHASE  EXPOSITION 

PRESENTED  WITH  THE  COMPLIMENTS 

OF  THE 

COMMITTEE  ON  MINES  AND  METALLURGY 

COMMITTEE 

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IKW*  v 


* 


I 


Copyright,  July  1904, 

By  The  University  of  Illinois. 


®ntbersttt>  of  JUmois 


Vol  I 


JULY,  1904 


No.  7 


Cl )f  Untorrsttg  grtutues 


The  Coals  of  Illinois;  Their  Composition 

and  Analysis 


S.  W.  PARR,  M,  S„ 

Professor  of  Applied  Chemistry  in  the  University  of  Illinois 


PRICE  25  CENTS 


(Hntbermtp  press 
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THE  COALS  OF  ILLINOIS. 

Their  Composition  and  Analysis. 

There  are  two  sources  of  motion  on  the  earth,  chemical 
action  and  gravity.  They  are  the  initial  forms  of  power  and 
constitute  the  prime  factors  in  industrial  development.  Their 
availability  in  any  region  is  an  index  of  present  or  potential 
activity.  Of  gravity  it  may  almost  be  said  that  it  has  become 
a  commodity  by  reason  of  its  easy  transformation  into  electric 
energy;  but  its  range  is  limited.  Chemical  energy  in  its  cheap¬ 
est  form  resides  in  the  coal  and  oil  deposits  of  the  world.  Their 
cost  of  transformation  is  the  great  problem  of  the  engineer. 
He  has  been  mainly  occupied  with  boilers  and  grates  and  stok¬ 
ers,  but  recently  a  marked  tendency  is  evident  towards  a  more 
critical  study  of  the  fuel  itself.  The  investigation  presented 
herewith  of  the  composition  and  properties  of  coal  is  a  con¬ 
tribution  in  that  direction. 

Geologically,  coal  is  a  mineral  derived  by  process  of  de¬ 
composition  from  organic  material  consisting,  in  the  main,  of 
cellulose.  We  know  the  products  of  decomposition  of  this 
material  when  submerged  to  be  carbon  dioxide,  marsh-gas  and 
water;  hence  a  chemical  change  takes  place  somewhat  after 
the  following  equation: 

6CeHioO  7  CCb  +  CLL  +  15H20  -f  (AsH^O 

Cellulose  Coal 

Now,  if  we  take  this  hypothetical  coal  molecule,  CmHkO, 
and  examine  it  chemically,  we  shall  find  that  under  the  influ¬ 
ence  of  heat  its  most  natural  decomposition  products  are  coke, 
marsh-gas  and  water,  indicated  in  an  equation  with  their  per¬ 
centages  as  follows  : 

C28H260  =  C22  -f-  6CH4  ~b  H2O 

Coal  Coke  Marsh-gas  Water 

100  per  cent.  —  69.84  per  cent.  +  25.40  per  cent.  +  4.76  per  cent. 

[291] 


4 


But  in  the  usual  method  of  analysis  a  separation  is  made 
between  the  coke,  or  non-volatile  part,  and  the  volatile  matter 
as  a  whole,  including  in  the  latter  both  the  marsh-gas  and 
water;  hence  we  have  a  procedure  represented  by  the  follow¬ 
ing  equation: 

C2sH‘260  “  C‘22  T  (6CH24  +  H2O) 

Coal  Coke  Volatile  Matter 

100  per  cent.  —  69.84  per  cent.  +  80.16  per  cent. 

This  volatile  matter  burns,  being  mostly  marsh-gas,  the 
chief  constituent  of  house-gas;  the  water  is  small  in  amount 
and  seems  to  have  been  in  a  measure  lost  sight  of,  for  this  vola¬ 
tile  material  came  to  have  the  name  “  volatile  combustible  ” 
applied  to  it.  Moreover,  water  of  more  genuine  characteristics 
is  always  found  present.  It  is  hygroscopic  and  invisible,  to  be 
sure,  but  it  can  be  removed  by  drying,  as  the  other  water  of 
composition  can  not  be,  and  hence  the  analysis  showing  only 
the  one  kind,  the  hygroscopic,  has  been  made  to  satisfy  both 
the  purpose  of  the  engineer  and  the  conscience  of  the  chemist. 
The  engineer  therefore  receives  his  results  in  percentages  of 
constituents  labeled  as  follows  : 

Ash 

Moisture 
Volatile  Matter 
Fixed  Carbon  or  Coke 

He  calls  the  first  two  the  non-combustible,  and  the  last  two 
the  combustible,  material;  and  to  the  sum  of  the  latter,  as  the 
unit  of  the  fuel,  he  refers  the  evaporative  efficiency  of  his 
boiler,  and  also  his  calorific  values,  on  the  theory  that  he  ob¬ 
tains  the  heat  units  per  pound  of  combustible  when  making 
the  calculation  to  the  material  as  “  ash  and  water  free.7’ 

Semi-Bituminous  Coal. 

In  the  accompanying  diagram  (Fig.  1)  the  characteristics 
of  this  type  of  coal  are  more  concisely  shown  and  in  the  rela¬ 
tive  proportions  of  the  constituents.  The  results,  moreover, 

[292] 


are  not  hypothetical,  as  above  considered,  but  are  taken  from 
ah  actual  sample  of  “  Pocahontas”  coal,1  which  belongs  to  the 
so-called  semi-bituminous  type,  and  constitutes  a  very  large 
part  of  the  coal  deposit  of  the  Appalachian  field. 

The  outer  zone  in  the  diagram  represents  the  constituents 
as  ordinarily  found  by  proximate  analysis,  and  in  tabular  form 
would  be  represented  thus  : 

Ash .  3.49  per  cent. 

Moisture .  .93  “  “ 

Volatile  Matter .  18.70  “  “ 

Fixed  Carbon .  76.88  “  “ 

100.00  “  “ 

Total  non-Combustible.  4.42  “  “ 

Total  Combustible  ....  95.58  “  “ 

Hence  104.62  pounds  of  coal  are  required  to  make  100.00 
pounds  of  actual  fuel. 

In  the  next  to  the  outer  zone  of  the  figure  the  constituents 
are  the  same,  except  that  the  “  volatile  matter  ”  is  subdivided 
into  that  part  which  in  our  hypothetical  coal  molecule  was 
referred  to  as  water  of  composition,  as  distinct  from  the 
“  moisture  ”  or  hygroscopic  water.  This  constituent  in  the 
actual  coal  amounts  to  4.21  per  cent.,  leaving  for  actual  com¬ 
bustible  in  the  volatile  part  only  14.50  per  cent,  instead  of  18.7 
per  cent,  as  before  indicated.  Hence  it  appears  that  our  report 
of  analysis  as  above  given  should  be  modified  to  read  thus  : 

Ash .  3.49  per  cent. 


Moisture . 

.93 

j  Water  of  Composition . 

4.21 

1  True  Volatile  Combustible. . 

14.50 

Fixed  Carbon . 

76.88 

100.00 

Total  non-Combustible . 

8.63 

Total  Combustible . 

91.38 

1  Trans.  Am.  Soc.  M.E.,  XXIV.,  1211. 

[293] 

ANALYSIS  -  EASTERN 

COALS 


Analysis  or  a  Semi-Bituminous  Coal 
(Pocahontas)  Showing  Constituents 
in  Relative  Proportions 

FIGURE  i. 

[294] 


7 


In  this  case  109.43  pounds  of  coal  are  required  to  make  100.00 
pounds  of  actual  fuel. 

The  inner  zone  of  the  diagram  shows  a  still  further  sub¬ 
division  of  the  true  volatile  combustible  into  carbon,  hydrogen 
and  sulphur;  but  of  this  subdivision  and  their  ratios  we  shall 
make  mention  later. 

The  type  of  coal  thus  far  considered  is  common  to  the 
Eastern  States  and  to  European  countries,  and  it  may  be  that 
analytical  processes,  at  least  the  so-called  “  proximate  analysis,” 
conveyed  an  element  of  untruth  of  not  sufficient  magnitude  to 
disturb  the  method  because  of  the  convenience  that  character¬ 
ized  it. 


Bituminous  Coal. 

Let  us  briefly  make  a  parallel  statement  concerning  the 
coals  of  the  Mississippi  Valley.  We  find  on  working  back  from 
the  present  structure  to  the  original  cellulose  decomposition, 
that  it  has  proceeded  somewhat  differently,  thus  : 


6C6H10O6  -  7C02  +  4CH4  +  13H20  +  CVJLsO, 

Cellulose  Coal 

The  decomposition  of  the  coal  in  analysis,  therefore,  would 
be  represented  thus  : 

C26H1802  =  C20  +  C6H12  +  3H20 

Coal  Coke  Pentane  Watt-r 

100  per  cent.  =  65.58  per  cent.  +  19.67  per  cent.  V  14.75 

To  carry  out  the  comparison,  a  second  diagram  has  been  pre¬ 
pared,  and  again  this  has  not  been  made  up  from  the  hypothet¬ 
ical  coal  molecule  just  presented,  but  from  the  average  of  results 
obtained  from  ten  typical  Illinois  coals. 

As  in  the  first  diagram,  the  outer  zone  represents  the  ordi¬ 
nary  proximate  analysis  and  by  the  usual  method  would  be 
reported  thus  : 


[2951 


ANALYSIS -ILLINOIS 

COALS 


Average  of  Ten  Illinois  Coals 
Showing  Constituents  in 
Relative  Proportions 


FIGURE  2. 
[296] 


°/V6V 


9 


Ash .  8.00  per  cent. 

Moisture .  7.00  •  “  “ 

Volatile  Matter .  35.60  “  “ 

Fixed  Carbon .  49.40  “  “ 

100.00  “  “ 

Total  non-Combustible.  15.00  “  “ 

Total  Combustible  ....  84.00  “  “ 

Here  we  need  119.00  pounds  of  coal  to  make  one  hundred 
pounds  of  fuel. 

The  next  zone  shows  the  relative  parts  when  a  division  is 
made  of  the  volatile  matter,  and  for  this  type  of  coal  the 
analytical  data  agree  somewhat  closely  with  our  hypothetical 
coal  molecule  given  above.  This  zone  shows  the  volatile  mat¬ 
ter  to  consist  of  14.00  per  cent,  of  inert  matter,  or,  as  we  have 
been  calling  it,  44  Water  of  Composition  ”,  and  21.6  per  cent,  of 
true  combustible  matter.  Hence,  instead  of  the  list  as  given 
above,  our  report  of  constituents  should  be  : 


Ash .  8.00  per  cent. 

Moisture .  7.00  “  “ 

\  Water  of  Composition .  14.00  “  “ 

)  True  Volatile  Combustible. .  21.60  “  44 

Fixed  Carbon .  49.40  “ 


100.00  “  “ 

Total  non-Combustible .  29.00  44  44 

Total  Combustible .  71.00  44  44 


Hence  there  are  required  141.00  pounds  of  coal  to  make  100.00 
pounds  of  actual  fuel,  instead  of  119.00,  as  by  the  usual  method. 

Lignite  or  Brown  Coal. 

It  is  of  interest  here  to  present  a  third  diagram  showing 
the  same  facts  ,with  regard  to  brown  coals,  a  North  Dakota 
lignite  being  used  for  the  analysis. 

[297] 


ANALYSIS OF  LIGh'ITIC 

COALS 


Analysis  or  a  Lignitic  or  Brown 
Coal  Showing  Constituents 
in  Relative  Proportions. 

FIGURE  3. 


[298] 


11 


By  reference  to  the  outer  circle,  which  represents  the  usual 
method  of  analysis,  we  have  results  as  follows  :• 

Ash .  2.71  per  cent. 

Moisture .  14.12  “  “ 

Volatile  Matter .  41.91  “  “ 

Fixed  Carbon .  41.26  “  “ 


100.00  “  “ 

Total  non-Combustible.  16.83  “  “ 

Total  Combustible  ....  83.17  “  “ 

Hence,  by  this  showing,  120.23  pounds  of  coal  would  be  re¬ 
quired  to  make  100.00  pounds  of  combustible. 

However,  upon  further  analysis  of  the  volatile  matter,  we 
find  it  to  consist  of  21.63  per  cent,  of  water  of  composition 
and  of  only  20.28  per  cent,  of  actual  combustible.  Hence  our 
results  should  be  made  to  read  as  follows  : 


Ash .  2.71  per  cent. 

Moisture .  14.12  “  “ 

S  Water  of  Composition .  21.63  “  “ 

l  True  Volatile  Combustible. .  20.28  “  “ 

Fixed  Carbon .  41.26  “  “ 


100.00  “  “ 

Total  non-Combustible .  38.46  “  “ 

Total  Actual  Combustible  . .  61.54  “  “ 


Here  there  would  be  needed  162.49  pounds  of  coal  to  make 
100.00  pounds  of  actual  combustible.  These  ratios  in  the  three 
types  of  coal,  with  the  differences  in  the  results  of  the  custom¬ 
ary  and  the  proposed  method  of  determining  actual  fuel,  may 
be  better  illustrated  in  a  table,  thus  : 


TABLE  i. 


No.  of  pounds  required  to  make  100  pounds 
of  “Combustible.” 

Error  of  common 
method  per  100 
pounds  of  actual 
fuel. 

Kind  of  Coal. 

Common  Method. 

Proposed  Method. 

Pocahontas  .  .  . 

104.62 

109.43 

4.81 

Illinois . 

119.00 

141.00 

22.00 

Lignite . 

120.23 

162.49 

42.26 

[209] 


12 


It  is  evident  from  the  table  that  a  boiler  rated,  for  example, 
at  an  efficiency  of  10  pounds  of  steam  per  pound  of  coal  of  the 
Pocahontas  ftype  would  have  difficulty  with  a  coal  wherein  22 
per  cent,  of  the  so-called  combustible  was  really  non-combusti¬ 
ble  and  inert,  to  say  nothing  of  the  loss  due  to  heat  of  vapor¬ 
ization  and  temperature  of  the  same  water  in  the  form  of 
escaping  flue  gases. 

Water  of  Composition  and  Volatile  Combustible. 

We  come  now  to  the  methods  for  obtaining  the  factors 
above  indicated.  At  first  thought,  an  ultimate  analysis  of  all 
the  constituents  would  seem  to  be  the  only  means  for  arriving 
at  these  data.  But  such  analyses  are  almost  prohibitive  for 
technical  use,  because  of  the  time  and  manipulative  skill 
involved;  but  more  than  this  it  may  be  questioned  whether  an 
ultimate  analysis  alone  will  give  the  data  in  the  desired  form. 
Very  much  depends  upon  the  factor  for  “  available  ”,  that  is, 
combustible,  hydrogen.  With  this  factor  at  hand,  and  one  for 
total  carbon,  we  have  all  the  constituents  that  can  enter  into 
the  actual  combustible,  with  the  possible  addition  of  a  small 
correction  for  sulphur. 

In  the  data  so  far  presented  the  factor  for  the  disposable 
hydrogen  has  been  calculated  from  the  results  obtained  by 
both  ultimate  and  proximate  analysis,  wherein  the  available 
hydrogen  in  bituminous  coals  was  regarded  as  a  part  of  the 
volatile  hydrocarbon  having  the  composition  represented  by 
the  formula  C6HI2,  or,  in  semi-bituminous  coals,  by  CH4.  The 
formula  in  each  case  therefore,  for  calculating  the  hydrogen 


would  be 
and  the 


C  and  Q-~-Cin  which  C  and  c  are  the  total  carbon 


5 


8 


fixed  carbon  respectively.  Therefore  (C  — c) 


C-c 


5 


would  represent  the  true  volatile  combustible,  and  this  value 
subtracted  from  the  total  volatile  matter  equals  the  water  of 
composition. 

Before  passing  to  the  consideration  of  methods  for  obtain¬ 
ing  the  total  and  fixed  carbon,  a  word  further  concerning  the 


[300J 


13 


deriving  of  hydrogen  from  these  constituents  is  necessary.  That 
this  method  is  applicable  to  certain  classes  of  coals  is  evident 
from  Table  II. 

Comparison  is  made  between  the  usual  method  for  arriving 
at  the  available  hydrogen  by  means  of  the  expression  (H — 


and  the  proposed  ratio  ( 


C 


The  first  results  are  derived 


from  the  averages  of  10  Illinois  coals.  The  others  are  calcu¬ 
lated  from  averages  obtained  by  Lord  and  Haas.1 

TABLE  II. 


Coals. 

% 

Percentage  of 
Available 
Hydrogen 

Difference 

in 

Percent¬ 

age. 

H — — 

8 

C  — c 

5 

Average  of  ten  Illinois  coals . 

3.76 

3.60 

—  .16 

Upper  Freeport,  Ohio  and  Penn. . . 

3.94 

4.20 

+  .26 

Pittsburg,  Penn . 

4.15 

4.28 

+  .13 

Darlington,  Penn . . 

4.10 

4.10 

.00 

Hocking  Valley,  Ohio . 

3.34 

3.67 

+  .33 

Thacker,  W.  Va . 

4.27 

4.39 

+  .12 

Pocahontas,  W.  Va.  (Sample  l)2. . . 

3.85 

3.35 

—  .50 

“  u  (Sample  2)2  ... 

3.97 

3.62 

—  .35 

From  the  table,  it  would  appear  that  the  possible  error 
from  thus  calculating  the  available  hydrogen  would  be  less 
than  one-half  of  one  per  cent,  of  the  true  value,  and  its  effect 
as  a  variable,  therefore,  in  calculating  the  true  volatile  com¬ 
bustible  would  fall  within  that  limit. 

It  may  not  be  concluded,  however,  that  so  uniform  a  ratio 
is  applicable  to  widely  varying  types  of  coal.  Indeed,  there  is 
good  evidence,  so  far  as  it  has  been  tested  in  connection  with 
Illinois  coals  at  least,  that  a  gradation  exists;  thus  if  we  let 
the  volatile  carbon  be  represented  by  total  carbon  minus  fixed 
carbon,  or  C  —  c;  then 


1  Trans.  Am.  Inst.  Min.  Eng.  XXVII.,  266-7. 


[301J 


14 


Where  C-c  =  10 

per  cent,  the  available  hydrogen 

—  1 

“  “  =15 

tt  it  gt  tt 

_  1 

- 4 

“  “  =20 

it  tt  tt  u 

_ _  1 

-  J 

“  “  =25 

tt  tt  a  a 

_ _  1 

—  ir 

A  diagram  therefore  has  been  arranged  as  follows  to  test  the 
correctness  of  the  above  ratios.  Fifty  Illinois  coals  have  been 
located  with  the  volatile  carbon  for  abscissa  and  that  amount 
of  hydrogen  for  ordinate  which  would  be  required  to  produce 
the  heat  values  indicated  by  the  calorimeter. 


FIGURE  4. 

Total  Carbon. 

It  will  be  noted  that  the  expression  — g-—  requires  the 

value  for  C,  that  is,  the  total  carbon  content  of  the  coal.  If 
this  must  be  obtained  by  the  usual  combustion  method  we  have 
made  but  little  progress  by  the  mere  development  of  the  above 
ratio.  It  is  proposed  to  obtain  the  factor  for  the  total  carbon 
by  means  of  the  apparatus  shown  in  Figure  5. 

Combustion  of  the  coal  is  effected  in  a  closed  bomb  as  in 
the  calorimetric  process  described  further  on,  by  use  of  sodium 

[302] 


15 


peroxide,  Na202,  the  product  of  the  combustion  being  sodium 
carbonate,  Na2C03.  The  solution  of  this  material  is  placed  in 
the  receptacle  A,  while  acid  is  in  B  and  C.  The  flask  C  con¬ 
tains  about  25cc.  of  sulphuric  acid,  and  a  carefully  measured 
volume  of  air  taken  at  common  pressure  and  temperature.  At 


Apparatus  for  "Total  Carbon  Determination. 

FIGURE  5. 

the  end,  after  admitting  all  the  carbonate  solution  and  meas¬ 
uring  the  volume  of  gas  evolved,  the  flask  C  is  completely 
filled  with  the  wash  water  from  A  and  the  total  volume  meas¬ 
ured  over  in  the  jacketed  pipette  PP.  By  subtracting  the 
initial  volume  in  the  flask  C,  the  exact  volume  of  carbon  diox- 

[303I 


16 


TABLE  III. 


[304] 


17 


ide  from  the  sodium  carbonate  is  obtained.  The  pressure  and 
temperature  readings  are  taken  and  from  the  subjoined  table 
the  exact  weight  of  the  carbon  is  derived.  Great  care  has  been 
exercised  in  the  preparation  of  the  table.  The  computations 
were  made  by  three  individuals,  with  comparison  of  results  to 
eliminate  all  possibility  of  errors  in  the  final  readings. 

Fixed  Carbon. 

It  will  be  evident  from  what  has  preceded  that  more  than 
usual  importance  attaches  to  the  factor  for  fixed  carbon.  A 
special  study  has  been  made  of  methods  for  obtaining  this 
factor,  first  because  the  method  recommended  by  the  commit¬ 
tee  of  the  American  Chemical  Society  on  coal  analysis1  is  not 
altogether  satisfactory;  and,  second,  because  with  western 
coals  high  in  sulphur  the  use  of  platinum  for  this  determina¬ 
tion  is  to  be  avoided  if  possible. 

The  report  of  the  committee  prescribes  heating  in  a  plati¬ 
num  crucible  over  a  Bunsen  flame  20  cm.  high  when  burning 
free.  Our  objections  to  the  prescribed  method  may  be  stated 
as  follows  •: 

The  heat  capacity  of  a  Bunsen  burner  is  not  measured 
alone  by  the  height  of  the  flame.  For  example,  a  large  sized 
adjustable  burner  with  a  tube  of  10  mm.  caliber  will  give  more 
heat  than  a  small  burner  with  a  tube  of  9  mm.  caliber,  and 
burning  at  the  regulation  height.  The  results  also  are  more 
variable  than  they  should  be.  This  is  more  noticeable  in  west¬ 
ern  than  in  eastern  coals,  but  in  any  case  it  is  to  be  expected 
that  the  platinum  crucible  arranged  as  prescribed  is  especially 
sensitive  to  external  influences,  and  especially  to  differences  in 
the  heat  capacity  of  the  flame.  In  the  table  following,  an  aver¬ 
age  sample  of  coal  designated  Sandoval,  Illinois,  was  used.  It 
cokes  freely,  and  has  ash  11.94  per  cent,  and  moisture  5.51  per 
cent,  Comparison  of  results  is  made  with  use  of  a  large  and 
small  sized  Bunsen  burner  as  above  described,  and  also  with 


[305J 


1  J.  Am.  Chem.  Soc.  XXL,  1122. 


18 


the  old  combination  of  burner  and  blast,  and  with  use  of  a 
porcelain  crucible  in  a  small  furnace  of  special  construction  to 
be  described  later. 

TABLE  IV. 


Determination  of  Volatile  Matter,  Sandoval,  Illinois,  Coal. 


Large  Bunsen  burner . 

• 

Highest  ...  . 

Lowest . 

35.71 

Flame  20  cm.  high . 

r 

Variation  . 

1.50 

Plat,  crucible,  Time  7  min.  . . . 

... 

H 

Average  of  eight  . . . 

36.52  per  cent. 

Small  Bunsen  burner . 

Flame  20  cm.  high . 

> 

Highest . 

Lowest . 

36.73  per  cent. 

35.69 

f 

Variation  . 

1.04 

Plat,  crucible,  Time  7  min . 

Average  of  eight .... 

36.13  per  cent. 

Bunsen  flame  31  min . . 

Blast  flame  min . 

-N 

\ 

r 

Highest . 

Lowest . 

Variation  . 

37.78  per  eent. 

36.53 

1.25 

Plat,  crucible . 

Average  of  fourteen. 

37.13  per  cent. 

Bunsen  flame  3£  min . 

N 

Highest . 

37.35  per  cent. 

Blast  flame  3£  min . 

Lowest . 

36.69 

Porcelain  crucible  in  special 

r 

Variation  . 

.66 

furnace  . 

Average  of  nine . 

37.10  per  cent. 

From  this  table  it  appears  feasible  to  replace  the  expensive 
platinum  crucible  with  one  of  porcelain.  The  serious  deterior¬ 
ation  of  platinum  under  the  combined  effect  of  red  hot  carbon 
and  sulphur  makes  this  end  a  very  desirable  one,  even  if  there 
were  no  advantage  in  the  results.  On  this  latter  point  there 
is  much  to  be  said  in  favor  of  the  porcelain  crucible.  The  in¬ 
itial  heating  up  is  somewhat  more  gradual.  A  bright  red  is 
very  easily  reached  and  evenly  maintained,  and  especially  is  it 
true  that  the  full  effect  of  the  heat  is  exerted  on  all  sides,  com¬ 
pletely  enveloping  the  crucible. 

The  form  of  apparatus  is  shown  in  the  accompanying 
figure. 

First,  as  to  the  lamp  :  This  simple  form  of  blast  lamp  has 
been  in  use  in  this  laboratory  for  the  past  seven  years,  and  has 

[306] 


19 


proved  itself  of  such  general  utility  as  to  merit  a  brief  descrip¬ 
tion. 

It  consists  essentially  of  a  Bunsen  burner  with  the  blast 
entering  at  the  usual  inlet  for  the  gas,  and  the  gas  entering 
through  a  side  tube  attached  where  the  air  is  ordinarily  ad¬ 
mitted.  The  air  is  discharged  through  a  tip  with  circular  open¬ 
ing  mm.  in  diameter,  and  is  so  adjusted  as  to  come  about 


even  with  the  lower  side  of  the  gas  inlet  tube.  A  wire  gauze 
is  inserted  in  the  tube  about  §  of  the  way  towards  the  top.  The 
lamp  is  especially  adapted  for  use  with  blast  of  constant  press¬ 
ure.  By  adjustment  of  the  air  it  may  be  made  to  burn  with  a 
common  Bunsen  flame.  In  connection  with  the  furnace  it  is 
allowed  to  burn  for  the  first  34  minutes  as  a  strong  Bunsen 
flame  of  12  inches  when  burning  free.  During  the  second 
period  of  3|  minutes  it  burns  as  a  blast  lamp.  The  combus- 

[307] 


20 


tion,  however,  leaves  the  tip  of  the  lamp  and  takes  place  en¬ 
tirely  within  the  chamber  underneath  the  crucible.  In  this 
way  an  excessive  amount  of  fuel  may  be  forced  into  a  small 
space  by  the  jet  action  of  the  blast.  The  combustion  taking 
place  in  this  chamber  and  the  hot  gases  being  turned  downward 
to  escape  through  the  annular  space  at  the  side,  a  very  intense 
heat  is  quickly  attained. 

A  cross  section  is  shown  through  the  furnace  in  Fig.  7. 


figure  7. 

The  base  B  rests  on  a  cast  plate  with  an  opening  1^  inches 
in  diameter.  The  crucible  rests  on  a  triangular  support  which 
permits  of  the  free  passage  of  the  gases,  part  of  which  may 
escape  through  a  small  opening  in  the  top  of  C,  but  mostly 
they  are  required  to  travel  downward  between  the  two  walls 
and  escape  at  the  lower  edge  of  R. 

A  common  glazed  crucible  of  Royal  Berlin  Porcelain  No. 
00  is  used.  Crucibles  as  true  as  possible  are  selected,  with  well 
fitting  covers,  and  these  are  ground  with  emery  powder  until 

[308] 


21 


the  lid  touches  at  all  points.  Crucibles  may  be  used  many 
times,  but  if  warping  occurs  the  covers  may  require  regrind¬ 
ing, — not  a  difficult  matter  and  easily  accomplished  by  hand  in 
five  or  ten  minutes. 

Sulphur. 

We  come  now  to  sulphur,  a  constituent  having  more  im¬ 
portance  than  is  usually  ascribed  to  it;  this  is  especially  true 
of  western  coals,  in  which  this  element  varies  from  1  per  cent, 
to  5  per  cent.  One  of  its  characteristics,  and  by  no  means 
the  least,  is  the  part  it  plays  as  a  disturbing  element  in 
nearly  all  the  determinations  in  coal  analysis.  The  Eschka 
method  is  satisfactory,  but  heat  other  than  from  a  gas  flame 
must  be  used.  There  is  still  some  question  as  to  the  like¬ 
lihood  of  sulphur  being  left  in  the  residue,  and  also  as  to 
the  necessity  of  dehydrating  the  silica.  The  use  of  sodium 
peroxide  as  an  oxidizing  agent  has  received  considerable  atten¬ 
tion,  but  the  violence  of  the  reaction  has  brought  disfavor  upon 
the  method.  However,  by  means  of  a  closed  bomb,  as  in  the 
Parr  calorimeter,  there  has  been  fully  demonstrated  the  prac¬ 
ticability  of  using  sodium  peroxide  for  this  purpose.  Indeed, 
over  two  years  ago,  Mr.  Milton  Hersey  of  Montreal,  Canada,  in 
a  communication  to  the  author  reported  the  very  satisfactory 
use  of  the  residues  from  the  calorimetric  process  for  gravimet- 
rically  determining  the  sulphur.  Later  articles  by  Sundstrom1 
and  by  von  Konek2  have  advocated  the  same  method. 

It  is  not  my  purpose  now  to  enter  into  a  discussion  of  this 
phase  of  the  matter,  but  simply  to  emphasize  the  fact  of  the 
completeness  of  the  oxidation,  which  has  been  verified  very 
many  times  by  the  writer. 

Coupling  the  sodium  peroxide  method  of  arriving  at  a 
combustion  with  the  photometric  method  proposed  by  Mr. 
Hinds,3  there  seem  to  be  possibilities  well  worth  investigating. 

1  Jour.  Am.  Chem.  Soc.  XXV.,  184. 

2  Zeit.  fiir  Ang.  Chem.  J903,  p.  517. 

3  Jour.  Am.  Chem.  Soc.  XXIII.,  269. 

[309] 


22 


The  work  with  the  photometer,  however,  either  as  outlined  by 
Mr.  Hinds,  or  as  elaborated  by  Mr.  Jackson,1  was  not  found 
satisfactory.  A  careful  study  was  made  of  the  variable  ele¬ 
ments  that  entered  into  the  proposition.  The  method  prescribed 
a  candle  of  standard  power,  maintained  at  a  definite  distance 
from  the  bottom  of  the  graduated  tube  in  which  was  read  the 
depth  of  liquid  through  which  the  outline  of  the  candle  flame 
could  be  seen.  It  was  soon  found  that  the  strength  of  the 
light  had  little  to  do  with  the  matter.  A  stronger  light  would 
illuminate  the  liquid  to  a  corresponding  degree  and  cause  the 
outline  of  the  candle  flame  to  disappear  at  about  the  same 
depth  as  a  lesser  light  with  a  less  illumination  of  the  liquid. 
As  between  a  common  candle  and  a  forty  candle  power 
acetylene  light  there  was  no  marked  difference.  Indeed,  the 
greatest  difference  was  noted  when  the  diffused  light  was  cut 
out  by  diaphragms,  in  which  case  the  light  could  be  seen 
through  a  greater  depth.  An  extreme  illustration  of  this  fact 
was  afforded  by  completely  blackening  an  incandescent  light 
bulb  and  then  cleaning  a  small  spot  to  show  a  short  length  of 
the  glowing  filament.  This  bit  of  filament,  which  afforded  no 
illumination  to  the  liquid,  could  be  seen  through  a  very  much 
greater  depth  than  was  the  case  with  an  ordinary  candle,  though 
its  power  was  far  below  the  standard.  Other  disturbing  conditions 
related  to  the  method  of  precipitation,  whether  hot  or  cold, 
whether  the  barium  salt  -  was  added  in  the  solid  or  the  liquid 
state,  whether  readings  were  made  at  once,  or  on  standing,  or 
whether  precipitations  made  in  the  cold  were  subsequently 
heated  or  not.  The  control  of  the  conditions  regarding  the 
light  has  been  accomplished  with  a  greatly  modified  apparatus 
in  the  following  manner,  as  shown  in  Fig.  8. 

The  tube  graduated  in  millimeters  is  placed  in  a  common 
flasly  having  a  little  clear  water  in  the  bottom.  The  flask  is 
placed  on  a  square  of  glass  resting  on  a  carbon  plate  about  §  of 
an  inch  thick  and  having  a  J  inch  hole  in  the  center.  The 

i  Jour.  Am  Cliem.  Soc.  XXIII.,  799. 

[310] 


23 


plate  is  adjusted  about  JO  inches  above  the  dame  of  a  common 
candle.  It  will  be  noticed  that  the  reading  tube  has  a  round 
bottom.  This  is  carefully  blown,  of  clear  glass  without  daw, 
and  ground  on  the  outer  surface;  the  whole  when  immersed 
playing  the  part  of  a  lens.  By  this  arrangement,  together  with 
the  diaphragm  effect  of  the  hole  in  the  carbon  plate,  a  pencil 
of  light  is  secured  with  the  minimum  amount  of  illumination 


Photometer  tor  Sulphur  Determinations. 

FIGURE  8. 

being  imparted  to  the  liquid.  Moreover,  instead  of  the  vary¬ 
ing  and  indednite  outline  of  a  candle  dame  there  appears  a 
steady  compact  point  of  light.  The  end  reading  is  thereby 
rendered  sharp  and  dednite.  It  is  interesting  to  note  that 
precipitations  made  with  the  barium  salt  in  solution,  or  with 
the  sulphate  solution  hot,  transmit  the  rays  from  the  candle  as 
white  light,  while  in  the  case  of  precipitations  made  with  the 
crystals  of  the  salt,  the  red  rays  only  are  transmitted,  the  illu- 

[311] 


24 


mination  of  the  liquid  is  in  this  way  still  further  reduced,  and 
the  sharpness  of  the  end  reading  is  thereby  promoted.  To 
secure  concordant  results,  definiteness  of  precipitation  must  be 
obtained.  This  is  accomplished  by  adding  the  barium  salt  to 
the  100  cc.  of  solution  at  room  temperature,  and  after  dissolving 
completely,  heat  on  the  water  bath  to  about  70°.  Let  stand 
for  half  an  hour  and  bring  to  the  room  temperature,  when  it  is 
ready  to  transfer  to  the  photometric  tube  for  reading.  With 
this  device  it  has  been  necessary  to  work  out  a  new  table.  (Ta¬ 
ble  VI).  The  conditions  are  purely  empirical,  but  not  arbitrary 
within  reasonable  limits,  except  as  to  the  size  of  the  hole  through 
the  plate  and  the  method  of  precipitation.  The  table  has  been 
developed  directly  from  a  standard  solution  of  potassium  sulphate 
having  5.4386  grams  dissolved  in  a  litre,  thus  containing  0.0001 
grams  of  sulphur  by  weight  per  cubic  centimeter  of  solution. 

Results  from  use  of  this  method  as  above  outlined,  in  com¬ 
parison  with  those  obtained  under  standard  conditions,  are 
shown  in  Table  V. 


table  v. 

Showing  Percentages  of  Sulphur. 


Illinois  Coal. 

Washings  from  Mahler 
Bomb. 

(Per  cent. ) 

Residues  from  Parr 
Calorimeter  in  Photo¬ 
meter. 

(Per  cent.) 

1.  Odin,  pea . 

2.30 

2.17 

2.  St.  John’s,  lump . 

1.55 

1.65 

3.  Pana,  slack . 

4.03 

4.04 

4.  Danville,  lump . 

2.16 

2.31 

5.  Ridgely,  pea .  . 

4.00 

4.01 

6.  Bloomington,  lump . 

2.57 

2.68 

7.  Spring  Valley,  washed . 

3.04 

3.20 

8.  Elmwood . 

1.53 

1.61 

With  this  form  of  apparatus,  the  facility  with  which  the 
sulphur  determinations  may  be  made  has  enabled  us  to  under¬ 
take  an  additional  factor  in  the  case  of  each  sample,  viz.,  the 
estimation  of  the  amount  of  sulphur  remaining  in  the  coke 
after  the  volatile  matter  has  been  driven  off.  The  coke  is  pul- 


[312] 


2 


o 


TABLE  VI. 


PHOTOMETRIC  TABLE  FOR  EULPHUR 

WEIGHT  OF  SULPHUR  IM  GRAMS 

PETR  MILLIMETER  DEPTH 

M.M 

SULPHUR 

IM  GRAMS 

M.M. 

SULPHUR 

IM  GRAMS 

M  M. 

SULPHUR 

IM  GRAMS 

M.M. 

SULPHUR 

IM  GRAMS 

200 

0.0  0/3  8 

/  5 1 

0.00/  61 

/  /  7 

0.00204 

83 

0.0027 0 

195 

0.00/4-0 

/50 

0.00/62 

H6 

0.00206 

82 

0.0 0273 

too 

0.0  0/42 

149 

0.00/63 

//5 

0.00208 

8/ 

0.002  77 

/  85 

0.00/45 

148 

0.00/64 

r/4 

0.00  2/0 

80 

0.0  0280 

183 

0  00147 

147 

0.  00/65 

//3 

0.002/2 

79 

0.0  0284 

/80 

0.00/50 

146 

0.0  0/66 

// 2 

0.002/4 

78 

0.00288 

/79 

0.0  0/50 

/45 

0.00/67 

III 

0.002/6 

77 

0.00292 

/78 

0.00/5/ 

/44 

0.00/68 

no 

0.002/8 

76 

0.0  0296 

/77 

0.00/5/ 

/43 

0.00/69 

J09 

0.0  0220 

75 

0.0  0300 

/76 

0.00/5/ 

}42 

0.00/ 7/ 

/08 

0.0022 2 

74 

0.00302 

/75 

0.00/5/ 

/ 4/ 

0.0  0/72 

/  07 

0.00224 

73 

0.00304 

/74 

0.00/52 

/ 40 

0.0  0/74 

706 

0.00  226 

72. 

0.00307 

773 

0.0  0/52 

139 

0.00/75 

105 

0.00  2  28 

7/ 

0.003/0 

/7Z 

0.00/52 

J38 

0  .00/76 

104 

0.00  230 

70 

0.0  03/3 

/ 7 / 

0.0  0/52 

/37 

0.00/77 

/  03 

0.00  23  / 

69 

0.003/7 

/  70 

0.00/53 

/  36 

0.00/79 

7 02 

0.00233 

68 

0.0  0320 

/62> 

0.00/53 

/35 

0.0  0/80 

10/ 

0.00234 

67 

0.00323 

/68 

0.00/53 

/34 

0.00/8  / 

/OO 

0.00  236 

66 

0.00327 

/67 

0.00/54 

/33 

0.00/82 

99 

0.00  238 

65 

0. 00330 

/56 

0.00/54 

J3  2 

0.00/84 

98 

0.00239 

64 

0.0  0335 

/65 

0  00/54 

/J  / 

0.00/85 

97 

0.00240 

63 

0.00340 

/64 

0.00/55 

/3  0 

0.00/87 

96 

0.0024/ 

62 

0.00345 

/63 

0.0  0/55 

/29 

0.00/88 

95 

0.00  243 

6/ 

0.00350 

/ez 

0.00/55 

128 

0.0  0/89 

94 

0.00  244 

60 

0.0  0355 

/6/ 

0.00/56 

/  2  7 

0.00/90 

93 

0.00  246 

59 

0.00360 

/ 60 

0.00/56 

/26 

0.00/9/ 

92 

0.0  0  248 

58 

0.00367 

/  59 

0.00/56 

/  25 

0.0  0/93 

9/ 

0.  OO  250 

57 

0.0  0373 

158 

0.00/57 

/  24 

0  .00  195 

90 

0.00252 

56 

0.0  0380 

/  57 

0.0  0/57 

/  23 

O.  0  0/96 

89 

0.00  255 

55 

0.00386 

/56 

0.00/58 

/22 

0.00/98 

88 

0.00  257 

54 

0.0  0393 

/55 

0.00/58 

/2I 

O.  0  0/99 

87 

0.00  260 

53 

0.0  0400 

/  5 4- 

0.00/59 

120 

0.0  0200 

86 

0.00  262 

52 

0.00407 

/S3 

0.0  0/59 

H9 

0.0020/ 

85 

0.0  0  265 

5/ 

0.004/3 

/5Z 

0.00/60 

!/8 

0.00203 

84 

0.00267 

50 

0.0  0420 

[313] 


26 


verized  and  burned  witli  sodium  peroxide  in  the  calorimeter 
bomb  as  usual,  and  the  sulphur  determined  in  the  residue  by 
means  of  the  photometer.  Having  determined  the  total 
sulphur  in  the  coal,  the  difference  between  these  two  factors 
represents  the  volatile  sulphur.  In  the  analytical  tables  at  the 
end  these  divisions  are  observed  tlnoughout. 

Calorific  Values. 

1st.  By  calculation  :  Many  attempts  have  been  made  to 
develop  a  reliable  formula  for  calculating  heat  values  from 
analytical  data.  The  formula  of  Dulong  is  the  most  reliable 
and  is  recommended  by  the  committee  of  the  A  merican  Chemical 

Society  in  the  following  form, 80S0C  +  84460  (H  —  ^)  +  2250S.1 

o 

The  variations  between  the  observed  calorific  values  and  the 
calculated  values  as  shown  in  Mahler’s  tables2  range  from  +  3 
per  cent,  to  —  3  per  cent.,  though  the  averages  of  numerous 
results  are  much  closer. 

The  variations  in  the  work  of  Lord  and  Haas  above  re¬ 
ferred  to  are  not  so  great,  ranging  from  -f  2  per  cent,  to  —  1.8 
per  cent.  Kent3  has  used  the  factors  3  and  5  times  the  avail¬ 
able  hydrogen  derived  from  ultimate  analysis  to  indicate  (when 
subtracted  from  the  total  carbon)  the  amount  of  fixed  carbon, 
and  to  the  various  percentages  of  fixed  carbon  he  has  assigned 
certain  calorific  values.  His  results  while  interesting  seem  to 
show  greater  conformity  in  the  case  of  eastern  than  of  western 
coals. 

Possibly  quite  as  good  as  any  method  of  calculation  would 
be  the  one  already  partially  suggested  in  the  discussion  con¬ 
cerning  the  derivation  of  the  factor  for  true  volatile  com- 


1  Jour.  Am.  Chem.  Soc.  XXL,  1130. 

2  Contributional  ’Etude  des  combustibles.  Mahler,  1892. 

3  Trans.  Am.  Inst.  Min.  Eng.,  XXVII.,  948. 


[314] 


27 


bustible  or  water  of  composition  (p.  IB).  Stated  as  a  formula 

it  would  be  8080C  +  34500  +  2250S  in  which  C  is  the 

0 

total  carbon,  c  the  fixed  carbon,  and  S  the  sulphur,  or  still 
more  accurately,  8080C  +  34500  (H)  -f  2250S,  wherein  H  is  the 
available  hydrogen  as  indicated  by  the  curve  in  Figure  4,  the 
point  being  located  by  the  percentage  constituent  of  volatile 
carbon  as  shown  by  C — c.  Calculated  in  this  manner  the  50 
Illinois  coals  there  listed  would  show  extreme  variations  from 
the  calorimeter  values  of  about  -f  1.5  per  cent,  to  —  1.5  per 
cent.  In  Table  VII.  the  calculated  results  thus  derived  are 
compared  with  observed  values  by  means  of  the  calorimeter. 

Concerning  calculations  in  general,  however,  it  is  well  to 
quote  Mahler1,  who  says  :  “We  cannot  give  a  general  formula 
depending  strictly  on  the  chemical  composition  which  will  give 
the  calorific  power  of  substances  so  complex  and  varied”;  or 
Poole,  who  says:2  “If  possible,  by  all  means,  have  a  calorimetric 
test.  If  not  possible,  use  the  best  analysis  available.” 

2nd.  By  observation:  The  calorimeter  devised  by  the 
writer  has  met  with  very  general  favor  and  is  now  widely  used 
both  in  this  country  and  abroad.  It  is  too  well  known  to  call 
for  detailed  description  here.  However,  a  few  modifications 
and  improvements  have  been  made  and  since  it  has  been  used 
in  the  accompanying  results  and  also  in  comparison  with  quite 
a  list  of  determinations  with  the  Mahler- Atwater  apparatus,  a 
brief  reference  is  here  given. 

Figure  9  shows  the  relative  positions  of  parts.  The  can  A. A. 
for  the  water  has  a  capacity  of  2  litres.  The  insulating  vessels 
B.B.  and  c.c.  are  of  indurated  fiber.  The  charge  of  coal  and 
chemical  are  put  in  the  cartridge  D.  Upon  ignition,  the  heat 
generated  is  imparted  to  the  water  and  the  rise  in  temperature 
is  indicated  on  the  finely  graduated  thermometer  T.  The  car¬ 
tridge  or  bomb  rests  on  the  pivot  F  and  is  made  to  revolve, 
thus  by  aid  of  the  small  turbine  wings  attached  effecting  a  com- 


1  As  quoted  by  Poole,  The  Calorific  Power  of  Fuels,  p.  io.  2  Ibid. 

[315] 


28 


plete  circulation  of  the  water  and  equalization  of  temperature. 

The  reaction  accompanying  the  combustion  may  be  repre¬ 
sented  by  the  equation: 

56N a202  +  C26Hi803  -  25  Na2C03  +  18  NaOH  +  22  Na20 

Sod.  perox.  Coal  Sod.  carb.  Sod.  hydrate  Sod.  oxide 

With  certain  substances  such  as  coke,  anthracites,  petrole¬ 
ums,  etc.,  a  more  strongly  or  vigorously  oxidizing  medium  is 


A 


FIGURE  9. 


needed  than  exists  in  the  peroxide  alone.  This  may  be  secured 
by  various  additions.  The  most  effective  are  a  mixture  of 
potassium  chlorate  and  nitrate  in  the  proportion  of  1  to  2  and 
this  mixture  used  in  the  ratio  of  1  to  10  of  the  sodium  peroxide; 
another  effective  mixture  is  an  addition  of  potassium  persul¬ 
phate  in  the  ratio  of  1  to  10  of  the  sodium  peroxide.  Other 

[316] 


29 


substances  facilitate  the  oxidation,  notably  ammonium  salts 
and  certain  organic  substances,  as  tartaric  or  oxalic  acid,  ben¬ 
zoic  acid,  etc.  In  the  work  on  Illinois  coals,  while  ordinarily 
no  extra  chemical  would  be  necessary,  still  in  certain  cases 
such  as  extra  slaty  coals  and  coals  with  excessive  volatile 

matter,  and  also  to  guard  against  variations  in 
the  quality  of  the  sodium  peroxide,  a  mixture 
as  first  described  above,  of  chlorate  and  ni¬ 
trate,  has  uniformly  been  used  throughout 
these  tests. 

One  peculiarity  in  the  behavior  of  the  com¬ 
bustion  has  been  improved  by  the  above  mix¬ 
tures.  This  behavior  is  probably  due  to  the 
fact  that  there  is  a  tendency  on  the  part  of  the 
particles  of  coal  in  immediate  contact  with 
the  metal,  which  is  kept  cold  by  exterior  con¬ 
tact  with  the  water,  to  escape  action  of  the 
chemical.  A  further  improvement  in  this 
particular  is  effected  by  a  modification  of  the 
bomb  as  illustrated  in  the  accompanying  fig¬ 
ure  (Figure  10).  The  air  space  about  the  low¬ 
er  part  of  the  bomb  prevents  direct  contact 
with  the  water.  However,  upon  ignition  this 
enclosed  air  expands  and  part  of  it  is  driven 
out  through  the  holes  below.  Later  as  cooling 
and  contraction  occur  the  water  is  drawn  into 
the  air  space  and  rapid  cooling  is  effected  but 
the  period  of  high  temperature  for  the  inter¬ 
ior  reaction  has  been  prolonged  from  a  few- 
seconds  to  a  half  minute  or  more.  Other  advantages  are  se¬ 
cured,  notably  the  avoidance  of  screw  threads  on  the  interior 
or  other  opportunity  for  material  to  lodge  and  cause  sticking 
or  difficult  removal  of  the  ends. 

In  Table  7  are  given  results  with  this  apparatus  in 

comparison  with  the  readings  obtained  by  use  of  a  Mahler- At¬ 
water  apparatus.  In  the  third  column  as  already  indicated 

[317] 


Calorimeter  Bomb 
FIGURE  10. 


TABLE  VII. 

Comparison  of  Calorific  Factors. 


No. 

Illinois  Coal. 

Mahler — 
Atwater  Bomb 
Calorimeter. 

Parr — 

Per-oxide 

Calorimeter. 

Calculation — 
8080  C  +  34500 
“H.” 

A 

Bloomington,  lump . 

6566 

6530 

6687 

B 

Carterville,  washed . 

7174 

7185 

7027 

C 

Danville,  lump . . . 

6797 

6762 

6804 

D 

Elmwood,  lump . 

7050 

6990 

7092 

E 

Moweaqua,  lump . 

6152 

6135 

6256 

F 

Odin,  pea . 

6227 

6257 

6333 

G 

Pana,  slack . 

5383 

5387 

5745 

H 

Ridgeley,  pea . 

5922 

5964 

6193 

I 

St.  Johns,  lump . 

6917 

6911 

6769 

J 

Spring  Valley,  washed . 

6150 

6109 

6346 

12 

Bloomington,  2nd  V.,  slack  . .  . 

5510 

5637 

5742 

13 

“  “  “  lump .... 

6447 

6511 

6571 

14 

“  3rd  V.,  slack.... 

6327 

6326 

6316 

15 

“  “  “  lump .... 

7140 

7106 

7119 

24 

Buxton,  lump . 

6534 

6520 

6540 

37 

Centralia,  slack . 

5911 

6020 

5879 

38 

Centralia,  nut . 

6425 

6476 

6440 

45 

Danville,  slack . 

6616 

6672 

6610 

60 

Eldorado,  slack . 

5743 

5777 

5854 

64 

Fairbury,  slack  . 

5782 

5868 

5893 

65 

1 1  lump . 

6804 

6747 

6773 

75 

Harrisburg,  lump . 

7370 

7379 

7276 

126 

Sandoval,  lump . 

6636 

6677 

6500 

131 

Springfield,  slack . 

6653 

6635 

6589 

134 

Streator,  2nd  V.,  slack . 

6343 

6395 

6371 

135 

“  “  “  lump . 

6962 

6983 

6948 

136 

“  7th  V.,  slack . 

6745 

6775 

6717 

137 

“  “  “  lump . 

7257 

7256 

7119 

140 

Trenton,  nut . 

5445 

5500 

5673 

141 

‘  ‘  slack  .  . 

5808 

5947 

6008 

under  “Calorimetric  Values  by  Calculation”  are  given  results 
obtained  by  use  of  the  formula  8080  C  +  34500  (H),  in  which  “H” 
is  the  percentage  of  available  hydrogen  as  indicated  by  the 
curve  in  Fig.  4.  The  samples  are  given  numbers  corresponding 
with  those  of  the  analytical  tables  at  the  end.  The  values  are 
given  in  calories  per  kilo.  (Cal.  per  kilo  x  1.8  =  B.T.U.  per 
pound). 

The  ultimate  analyses  which  have  served  as  the  basis  for 
some  of  the  preceding  calculations  are  embodied  in  Table 
VIII.  There  is  also  included  the  proximate  analyses  and  a 
comparison  of  values  obtained  by  the  old  and  new  methods 

Results  are  given  throughout  in  per  cent. 

[318] 


TABLE  VIII. 


31 


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[3i9] 


32 


The  samples  for  Table  IX.  were  collected  between  Feb.  8th 
and  June  8th,  1904.  These  were  obtained  at  the  mines  from 
the  surface  of  car  lots  as  made  ready  for  shipment  to  the  con¬ 
sumer.  Amounts  varying  from  40  to  50  pounds  were  taken 
and  shipped  in  sacks  to  the  laboratory.  In  general  one  sample 
of  lump  or  screened  nut  and  one  of  screenings  or  slack  was 
procured  from  each  mine.  The  term  “  slack  ”  has  been  uni¬ 
formly  applied  where  the  material  included  all  that  passed 
through  a  1^  inch  screen. 

Immediately  upon  receipt  of  the  material  it  was  reduced 
by  quartering  in  the  usual  manner.  A  check  sample,  buck¬ 
wheat  size,  was  taken,  another  part  was  ground  to  passthrough 
a  100  mesh  sieve  and  each  was  sealed  in  a  “  lightning  ”  fruit 
jar.  The  analytical  results  are  given  in  per  cent.  The  calorific 
values  are  given  in  British  thermal  units  per  pound  of  actual 
coal  as  represented  by  the  samples  and  also  in  calories  per  kilo 
of  actual  coal. 


[Note. — For  the  collection  of  many  of  the  samples  I  am  indebted  to  the  State 
Mine  Inspectors,  and  I  wish  here  to  express  my  appreciation  of  their  interest  and 
efficiency.  The  general  analytical  work  has  been  in  charge  of  C.  H.  McClure,  assist¬ 
ed  by  Chas.  Edwards  and  A.  C.  Brown,  and  I  heartily  commend  the  skill  and  faith¬ 
fulness  which  has  characterized  their  part  of  the  work. — S.  W.  P.] 


[32o] 


Chemical  Analyses  and  Heating  Valles  of  Illinois  Coals. 


33 


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[324] 


TABLE  IX— Continued. 

Chemical  Analyses  and  Heating  Values  of  Illinois  Coals. 


37 


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a 

2 

a 

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S 

be 

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c3 

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B 

s 

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a 

a 

a 

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O 

O 

O 

O 

dn 

a 

a 

2 

2 

Ph 

5a 

7} 

r/a 

7? 

m 

aa 

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a 

c3 

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•joqiunjsi 


00  05 


O  rH 
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M 

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CO  r* 
(M  M 


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M 


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CO 


CO 


01 

CO 


co 


[327] 


TABLE  IX— Continued 

Chemical  Analyses  and  Heating  ArALUES  of  Illinois  Coals. 


40 


tri 

ro 

CO 

CO 

40 

CD 

O 

CO 

rH 

GO 

xH 

GO 

rH 

rH 

05 

CO 

rH 

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O 

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1  — 

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40 

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05 

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05 

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05 

CD 

CD 

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4-5 

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05 

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CO  0 

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40 

xH 

O 

CD 

a 

p 

CD 

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CD 

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40 

CD 

CD 

CD 

CD 

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CD 

40 

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t 

40 

1- 

40 

40 

■»— 1 

O 

40 

CD 

rH 

05 

O 

05 

05 

rH 

Cl 

05 

CO 

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0 

05 

CO 

CO 

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05 

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Cl 

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l- 

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rH 

40 

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40 

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05 

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paxt^[ 

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[32S] 


NUMBERS  OF  THE  UNIVERSITY  STUDIES  PREVIOUSLY 

ISSUED 


[Address  all  communications  concerning  the  Studies  to  Editor,  University  Studies, 
305  University  Hall,  Urbana,  Ill.] 

Yol.  1.,  No.  1.  Abraham  Lincoln  :  The  Evolution  of  his  Literary  Style.  By  Pro¬ 
fessor  D.  K.  Dodge,  Ph.D. 

No.  2.  The  Decline  of  the  Commerce  of  the  Port  of  New  York.  By  Mr. 
Bichard  Price  Morgan. 

No.  3.  A  Statistical  Study  of  Illinois  High  Schools.  By  Mr.  F.  G.  Bonser,  M.S. 
No.  4.  The  Genesis  of  the  Grand  Bemonstrance  from  Parliament  to  King 
Charles  I.  By  Henry  Lawrence  Schoolcraft,  Ph.D. 

No.  5.  The  Artificial  Method  for  Determining  the  Ease  and  the  Bapidity  of 
the  Digestion  of  Meats.  By  Harry  Sands  Grindlev,  Sc.D.,  and 
Timothy  Mojonnier,  M.S. 

No.  6.  Illinois  Bailway  Legislation  and  Commission  Control  since  1870.  By 
Joseph  Hinckley  Gordon,  A.  M.  Introduction  by  Professor  M.  B. 
Hammond,  Ph.  D. 


